# A 30.00 mL sample of an unknown H3PO4 solution is titrated ## Problem 88E Chapter 4

Chemistry: A Molecular Approach | 3rd Edition

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Problem 88E

A 30.00 mL sample of an unknown H3PO4 solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 mL of NaOH solution is added. What is the concentration of the unknown H3PO4 solution? The neutralization reaction is Step-by-Step Solution:
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Solution: Here, we are going to write a balanced chemical equation for the given reaction and calculate the concentration of the remaining ions. Also, we are going to determine whether the resultant solution is acidic or basic. Step1: a) When a solution of 15.0 g of Sr(OH) is mixed with 2solution of 255.0 ml of 0.200 M HN0 , strontium nitrate and water are formed. The balanced chemical equation for the 3 above reaction is given below: Sr(OH) (a2 + 2HN0 (aq) --3---> Sr(N0 ) (aq) + 23 2 2 Step2: b) Given mass of Sr(OH) = 15.0 g 2 Molar mass of Sr(OH) = 121.6 g/ mol 2 Therefore, number of moles of Sr(OH) = 15.0 / 121.62 = 0.123 mol Again, number of moles of HN0 = Volume of s3ution in litres X Molarity = (55 / 1000 L) X 0.200 M = 0.055 L X 0.200 M = 0.011 mol From the equation given above, it is clear that 2 moles of HN0 reacts with 1 mole o3Sr(OH) . 2 Therefore, 0.011 mol of HN0 will react with (0.011 / 2 = 0.0055) mol of...

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##### ISBN: 9780321809247

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A 30.00 mL sample of an unknown H3PO4 solution is titrated

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